Topic 2- atomic structure and bonding Flashcards
Fill in table
Particle Relative mass Relative charge Location
Proton
Neutron
Electron
1, +1, nucleus
1, 0, nucleus
1/1840, -1, shell
What is an isotopes
Has the same number of protons but different number of neutrons therefore a different mass
What is the Relative atomic mass
The average mass e.g. For chlorine
(75x35)+(25x37)/ 100= 35.5
What is the plum pudding model
Label it
Who proposed the idea
The structure of an atom
It had a positive sphere ans negative electrons
J.J. Thompson
Groups go ______ and periods go _______ in the periodic table
Down and across
How many electron in group fives outer shell
Five
What is a positive ion called
What is a negative ion called
Cation
Anion
How is an ion formed
When an atom loses or gains an electron to gain a full outer shell
Simple negative ions change the end of their names to…
ide
Eg. Chloride
What is a molecular molecule
Contains more than one atom and are charged particles
What happens in a ionic bond
When there is a transfer of electrons to form a full outer shell
The attraction of oppositely charged ions
Ionic compounds do not have a _______ but the ions do have a _____
Charge
What is the formula of sodium chloride Calcium chloride Magnesium oxide Potassium sulfite NOTE* group number/ valency will help
NaCl
CaCl2
MgO
K2S
What are subatomic particles?
Electrons, protons, neutrons
What are the properties of ionic compounds (6)
1) . High melting and boiling points
2) . Cannot conduct electricity when solid
3) . Can conduct electricity when liquid/ molten
4) . Lots of energy required to break down the forces of attraction
5) . Solid at room temperatures
6) . Most compounds can dissolve in liquids making them aqueous
Covalent bonding
Between two or more non-metals
Shared pair of electrons
What is a diatomic molecule
They exist as molecules
Containing two atoms covalently bonded together
Write the covalent bond of
Hydrogen
Chlorine
Oxygen
H-H
Cl-Cl
O=O
What are the properties of simple covalent substance
Doesn’t conduct electricity
Usually gas or liquid at room temperature
Doesn’t electricity because no charged particles
Has weak forces of attraction, van dear Waals
Insoluble in water
Give two examples of giant covalent substances
What element do they share in common?
Graphite and diamond
Carbon
What is an allotrope
Give two examples
Different forms of the same element with the same physical state
Give the properties of diamond
Carbon atom joined to four other carbon atoms
Tetrahedral
Has strong bonds between atoms, strong covalent atoms
Doesn’t conduct electricity because there are no free delocalised
electrons
High melting and boiling points
Insoluble in water
What is diamond used for and give a reason
For cutting materials such as enamel (hardest substance in body) because diamond is the hardest substance on earth due it its tetrahedral shape
Give the properties of graphite
Has strong covalent bonds between atoms
Has weak bonds between layers because of free delocalised electron
Joined to three other carbon atoms
Insoluble in water
Can conduct electricity
Cannot conduct electricity when molten/ liquid because structure is ruined
High melting and boiling points
What is graphite used for
A lubricant because the weak force of attraction between the layers, due to a free delocalised electron, lets the layers slide over each other.
Metallic bonding is caused by the _______ between _______ _______ and _______ ______ in the structure of the metal
Attraction
Delocalised electrons
Positive metal ions
What is an alloy
Is a mixture of two or more elements which at least one is a metal eg. Brass
What is ... used for Aluminium Copper Iron Magnesium
Overhead power cables because of low density and good conductor of electricity
Electrical wires because of being a good conductor of electricity
For bridge and building because of high density and high melting and boiling points
For flares because it burns with a bright white light and also for strong alloys in aircraft because of low density
